Metals useually have few valence electrons and they loose electrons from their outermost shell thus, forming an ion with positive charge (cations). This is because it is easy for metals to loose electron and attain stable or octet configuration similar to rare gases. Hence to attain stability metals lose valence electrons. E.g. sodium (At no. =11 ; electronic configu-1s2, 2s2, 2p6, 3s1) metal has one valence electron and it is easy for it to loose 1e rather to gain 7e to attain stable configuration. Hence it loose 1e forming Na+ cation.
Metals are those elements which have large atomic sizes and low I.P values and also 1 to 3 electrons in outermost shell so they easily donate the electrons for their stability.
they borrow
In a ionic bond, which is a bond between metals and nonmetals, the metal will loose the electron(s) while the nonmetal will gain the electron(s).
Ionisation energy determines the ability to loose electron. It tells the amount of energy changes in the process.
The metal gives its electron(s) to a nonmetal.
In ionic bonding, the metal loses the electron forming the cation and the non metal gains that electron forming the anion
we make use of tungsten metal to design electron gun.
Since it has 1 valence electrons it is a metal and also non metal because it may loose 1 electron to stabilize or also gain 1 electron to stabilize. Metals loose electrons and non-metals gain electron and hydrogen have both metallic (to loose) and non-metallic (to gain) properties.
In a ionic bond, which is a bond between metals and nonmetals, the metal will loose the electron(s) while the nonmetal will gain the electron(s).
alkali metals need to loose one electron. alkali earth metals need to loose two
In order for an electron to be ejected from a metal surface, the electron must be struck by a photon with at least the minimum energy needed to knock the electron loose.
I assume you are talking about the Alkali metal group which in fact would readily loose their outer electron to form a 1+ cation (have a full valence electron shell).
Metals which can easily loose electron are most reactive. They are present in group-1.
Ionisation energy determines the ability to loose electron. It tells the amount of energy changes in the process.
Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
This electron is the only one in a new outermost electron shell as you progress through the periodic table. So it is relatively easy for it to hop off and join to a Chlorine atom, for example, which is one short of a completed shell. So it's good in forming ionic compounds,
The metal gives its electron(s) to a nonmetal.
The Alkali Metals loose one electron in order to achieve a nobel gas configuration.
Hydrogen has 1 electron. It can easily gain or lose electron to form metal or non metal